Ionic Equilibrium
Chemical equilibrium and ionic equilibrium are two major concepts in chemistry. Ionic equilibrium deals with the equilibrium involved in an ionization process while chemical equilibrium deals with the equilibrium during a chemical change. Ionic equilibrium is established between the ions and unionized species in a system. Understanding the concept of ionic equilibrium is very important to answer the questions related to certain chemical reactions in chemistry.
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Bronsted Lowry Base In Inorganic Chemistry
Bronsted-Lowry base in inorganic chemistry is any chemical substance that can accept a proton from the other chemical substance it is reacting with.
![The molar solubility of silver carbonate in a 0.165 M potassium carbonate solution is 7.78x10^-7
М.
Incorrect
K2CO3 is a soluble salt. Ag,C03 is not.
The solubility of Ag,CO3 in pure water is 1.3x10 4 M. The solubility of Ag,CO3 will be less than this
in the presence of potassium carbonate, because there is already CO3²- ion present in the solution.
This is known as the "Common Ion Effect".
Initial [CO2 ] = 0.165 M from the K2CO3 solution.
Step 1: Set up the equilibrium using the ICE method
Let 's' = number of moles of Ag2CO3 (s) per liter that dissolves = molar solubility
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Ag2C03 (s) = 2Ag* (aq) +
Co3² (aq)
Initial
some
0.165 M
Change
Equilibrium
+ 2s
some
+ 2s
0.165 +s](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0a4e7880-3731-4736-9087-0e959d4f3aa8%2F05266efe-8946-494d-97fd-b3aea67dd5c1%2Fatc5iz_processed.jpeg&w=3840&q=75)
![A92CO3 (s) = 2Ag* (aq) +
Co,² (aq)
Initial
some
0.165 M
Change
Equilibrium
S
+ 2s
some
+ 2s
0.165 + s
Setp 2: Substitute the equilibrium values into the the Ksp expression
Ksp =[Ag*]? [CO3²] =(2s)?(0.165 + s) = (from the table)
8.1×10 12
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Step 3: Assume that s is small relative to 0.165 M, so that the approximation 0.165 + s 0.165 can
be made. This is reasonable because the solubility is low without the common ion and it will be even
lower in the presense of added CO3?. Then:
Ksp = (2s)2(0.165) = 8.1×10 12
%3D
%3D
Step 4: Solve for s
Ksp
(1/2)
(1/2)
:(
8.1x10-12
s= (1/2)
(1/2)
3.5×10 6 M
%3D
(0.165)
(0.165)
Step 5: Check the approximation:
Next
0.165 + S
0.165 + (3.5×10-6)
0.165
0.165
OK
%3D](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0a4e7880-3731-4736-9087-0e959d4f3aa8%2F05266efe-8946-494d-97fd-b3aea67dd5c1%2F7ofm7z_processed.jpeg&w=3840&q=75)
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